For the reaction
CH3OHsld 1 32
O2sgdh2H2Osld 1 CO2sgd
the value of ΔG ° is −702.2 kJ at 25°C. Other data are as
follows:
DHf 8 (kJ/mol) S 8(J/mol∙K) at 258C at 258C
CH3OH(l ) −238.7 126.8
H2O(l ) −285.8 70.0
CO2(g) −393.5 213.7
Calculate the standard entropy, S °, per mole of O2(g).
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For the reaction CH3OHsld 1 32 O2sgdh2H2Osld 1 CO2sgd the value of ΔG ° is −702.2...
1. 1) luciferin+O2 ⇌ oxyluciferin+light 2) ATP⇌AMP+PPi ΔG∘=−31.6 kJ/mol If the overall ΔG∘ of the coupled reaction is -1.21 kJ/mol , what is the equilibrium constant, K, of the first reaction at 11∘C? Round your answer to 3 significant figures. 2. When methanol (CH3OH) is combusted, such as when in a gasoline blend, the following reaction occurs: 2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(g) Based on the standard free energies of formation given, what is the standard free energy change for this reaction? Report the answer...
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Calculate the ΔG°rxn at 298 K using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K 146.0 210.8 240.1 70.0
The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) → C2H6(g) ΔH = −84.0 kJ/mol
At 298 K, evaluate deltaG(kJ) and deltaE (V) for 2CH3OH(l) + 3O2(g) -> 4H2O(g) + 2CO2(g) S (J/mol-K) AH°y (kJ/mol) So (J/mol-K) AH(kJ/mol) Substance Substance N2(g) CH-ОН() 126.8 0 191.5 -238.6 CO(g) NH3(g) 197.9 192.5 -110.5 -46.2 CO2(g) NO(g) 213.6 +90.4 210.6 -393.5 NO2(g) +33.8 240.5 H2(g) HNO3(aq) 130.6 146.0 -206.6 H2O( 69.9 -285.8 O2(g) 188.8 H2O(g) 0 205.0 -241.8
Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K 146.0 210.8 240.1 70.0 -151 kJ +50.8 kJ -186 kJ +222 kJ -85.5 kJ
Methanol, CH3OH (l), combusts according to the following equation: 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l) ∆rHo (298 K) = −1452 kJ Here is a list of Entropies of formation: S (J K-1 mol-1) at 298 K CH3OH (l) =126.8 O2 (g) = 205.14 CO2 (g) = 213.74 H2O = (l) 69.91 (a) If the above reaction was used in a fuel cell, say, to perform work, what will be the maximum...
Calculate the entropy of the following reaction, using the table below. Enter your answer without units to one decimal. 2C6H6(g) + 15O2 (g) → 12CO2 (g) + 6H2O (g) Substance ΔHf° (kJ/mol) ΔGf° (kJ/mol) S° (J/mol∙K) CH3COOH (g) -484.3 -389.9 159.8 (CH3)2O (g) -184.1 -112.6 266.4 C2H6 (g) -84.0 -32.0 229.2 C2H5OH (g) -234.8 -167.9 281.6 C6H6 (g) 82.9 129.7 269.2 CO2 (g) -393.5 -394.4 213.8 H2O (g) -241.8 -228.6 188.8 H2O (l) -285.8 -237.1 70 O2 (g) 0.0 0.0...
Consider the reaction 2 CO2(g) +5 H2(e) C H2(e) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: Submit Answer Retry Entire Group more group attempts remaining AH,(kJ/mol) AG® (kJ/mol) Sº (J/mol K) -238.7 -116.0 126.8 219.0 -363.0 249.0 135.1 -166.3 -110.0 -351.0 125.0 209.2 68.2 - 129.0 202.0 226.7 200.9 52.3 - 166.0 -53.0 -277.7 219.6 250.0 242.0 160.7 -13.0 -235.1 282.7 Carbon CH3OH (1) H2CO...
The change in Hrxn for the reaction C8H8 + 10 O2 = 8 CO2 + 4 H2O is -4395 kJ/mol. Knowing this, as well as the standard enthalpies of formation below, calculate the standard enthalpy of formation of Styrene in kJ/mol. change in Hf[CO2 (g)] = -393.5 kJ/mol change in Hf[H2O (l)] = -285.8 kJ/mol